1. Draw the MO diagram for HBr. The orbital potential energies for the 4s and 4p of Br are -18.65 ev and -12.49ev, respectively. Recall that the H 1s is -13.61ev.
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1. Draw the MO diagram for HBr. The orbital potential energies for the 4s and 4p of Br are -18.65 ev and -12.49ev, respectively. Recall that the H 1s is -13.61ev.
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- How many valence electron does Br haveQ2) Consider the following atoms: a- CI, Ga, Br, P, S and Si What is the effective nuclear charge for each atom? b- What are the possible quantum numbers for n=1, n=2 and n=3? Q3) What are the orbital hybridization for each of the following: Explain 1- BCI, 2- C,H. 3- Cr(CO), 4- Fe(CO), 5- CH, 6- PtBr,Use the data given below to calculate the bond energies (Do) (in eV) of 'H³°CI and 'H®l Br molecules. Which bond is stronger? Molecule ve (cm=1) De((cm¯1) HCI 2991 53194 HBr 2649 34570
- Huckel theory: All atomic orbital coefficients in the lowest energy MO (Ψ1) should have the same value – explain why?33W.) In dative bonding, two electrons are being transferred in one atom to forma bondX.) Battery-operated cars emit carbon dioxideY.) Clockwise rotation of electron is designated as arrow downZ.) Helium has its valence electron in the p orbitalA.) If all 4 statements are trueB.) If 3 of the 4 statements are trueC.) If 2 of the 4 statements are trueD.) If only 1 of the 4 statements is trueE.) If none of the 4 statements is true44. The molecule H3* has long been speculated to exist. The interest here is that the addition of the smallest bit of nuclear matter, a proton, now introduces additional nuclear repulsion over the H₂ problem. The issue was whether electron distributions could lead to a stable configuration. a) Draw what you think would be the most stable structure for H3* and show all the Coulombic terms (write out the potential needed for the corresponding Schroedinger equation). b) Draw what you think is the least stable configure of the 3 protons and 2 electrons. c) It is found that the structure involves the rotation of one proton around the other two, and interchange of which proton is rotating. Offer a potential explanation (think tunneling).
- 4. Molecular Orbital Theory Let's construct an MO diagram for KrBr*, the krypton bromide cation. Let's focus only on the n=4 valence shell in for both species. a) Which of the two atoms, Kr or Br, has a 4p electrons that are lower in energy? Justify your answer in terms of periodic trends. Also provide experimental evidence for your answer in terms of ionization energies (available online). b) Based on part (a), draw an MO diagram for KrBr*, reflecting the appropriate relative energies of the Kr/Br valence electrons. Connect the orbitals that mix/split with dashed lines. c) Populate the MO diagram with the appropriate number of valence electrons. What is the expected bond order?Use the data given below to calculate the bond energies (Do) (in eV) of1H35Cl and 1H81Br molecules. Which bond is stronger? HCl Ve (cm^-1): 2991, De(cm^-1): 53194 HBr Ve(cm^-1):2649 , De(cm^-1): 34570Consider a ring system made up of 8 atoms (each one contributing a p atomic orbital to make 8 pi molecular orbitals). If the system is filled with 6 orbitals containing single, electrons, there will 6 orbitals containing pairs of electrons and 1 unpaired electrons. Hint: Use a Frost Circle. Use numbers rather than text for your answers.
- Write down the uncondensed electronic configurations for Co;; Co2+ and Co3+. In the case of the Co2+, which orbital is losing electrons? Why is this the case?Bro 1) The orbital potential energies for the 4s and 4p of Br are -18.65 ev and -12.49ev, respectively. Recall that the H 1s is -13.61ev. The MO diagram for HBr is not exactly the same as HF. Draw the MO diagram for HBr, including energy levels, each orbitals shape, each orbitals character (meaning what atomic orbitals contribute to each M.O. and how much), symmetry labels (e.g. o and t, o* and a*), indicate the HOMO and LUMO, the bond order (show your work), whether the molecule is paramagnetic or diamagnetic. NowRelate the energies of the orbitals found (these we will use for building Molecular Orbital energy level diagrams) to Z*, also known as Zeff, determined by Slater’s rules Please show calculations for the following: H (1s electron) He (1s electron)